Directions:
a) list and define all vocabulary from the chapter
b) type at least 4 sample problems with step-by-step directions of how to solve the problem; list the correct answers (if your chapter doesn't have math, there are still problems and concepts we learned.)
c) link at least 3 websites for additional resources to help with studying
d) develop your own LEQ questions for the section - what did you think were the key points we learned?
e) Once your page is done, visit 4 other chapters and answer their LEQ's. (This can be done on a separate piece of paper)
a.) LEQ: How can I draw a bond using electrons? How can I name a covalent bond?
Lewis Dot Structure- element symbol that represents the nucleus, inner electrons, & surrounding dot represent the valence electrons
Electron pairs- two electrons that occupy the same orbital but have different spins
Single bond- Shares two electrons; single bonding pair of electrons
Double bond- shares 4 electrons; two bonding electron pairs
Triple bond- shares 6 electrons; three bonding pairs
Binary covalent- the combination of two elements, usually nonmetals
Bromine has three electron pairs & 1 lone electron; it needs only one more electron to become stable
Chlorine also only needs one more electron to become stable
Aluminum has three lone electrons, so to become stable it needs to bond three different times
Oxygen has two electron pairs & 2 lone pairs; it needs to bond two times to become stable
LEQ: How can I classify a bond type?
Electronegativity- how strong bonds are within a compound
Ionic bond- bonds between metals & non-metals; atoms with large differences in their tendencies to lose or gain electorns
Covalent bond- bonds between nonmetals & non-metals; atoms that have small differences in their tendencies to lose or gain electrons
Metallic bond- bonds between metals & metals; lose their valence electrons but do not gain them, so the electrons "flow" between the atoms (back & forth)
Polar- unequal distribution of electron density, the bond has partial negative & partial positive poles
Non-polar- atoms are identical, bonding pair is share equally
Organic compound- carbon is nearly always bonded to itself and hydrogen & often to other elements
Inorganic compound- any compund that does not contain carbon
Intermolecular force- the atrractive & repulsive forces among patricles in a sample of matter
This is an ionic bond because Na is a metal with only one electron & it bonds with Chlorine, a non-metal, who needs only one more elctron to have a full outershell
This is a covalent bond because they are both non-metals
LEQ: How can I predict the 3-D shape of molecules?
Linear- 0 unbonded pairs around the central element
2 locations bonded to central
Hybridization: sp
Trigonal Planar- 0 unbonded pairs around central element
3 locations bonded to central
Hybridization: sp2
Bent- 2 unbonded paris around central element
2 locations bonded to central
Hybridization: sp3
Pyramidal- 1 unbonded pari around central element
3 locations bonded to central
Hybridization: sp3
Tetrahedral- 0 unbonded pairs around central element
4 locations bonded to central
Hybridization: sp3
Bond angle- the angle formed by the nuclei of two surrounding atoms with nucleus of the central atom at the vertex
a) list and define all vocabulary from the chapter
b) type at least 4 sample problems with step-by-step directions of how to solve the problem; list the correct answers (if your chapter doesn't have math, there are still problems and concepts we learned.)
c) link at least 3 websites for additional resources to help with studying
d) develop your own LEQ questions for the section - what did you think were the key points we learned?
e) Once your page is done, visit 4 other chapters and answer their LEQ's. (This can be done on a separate piece of paper)
a.) LEQ: How can I draw a bond using electrons? How can I name a covalent bond?
Lewis Dot Structure- element symbol that represents the nucleus, inner electrons, & surrounding dot represent the valence electrons
Electron pairs- two electrons that occupy the same orbital but have different spins
Single bond- Shares two electrons; single bonding pair of electrons
Double bond- shares 4 electrons; two bonding electron pairs
Triple bond- shares 6 electrons; three bonding pairs
Binary covalent- the combination of two elements, usually nonmetals
http://www.ausetute.com.au/lewisstr.html
http://hyperphysics.phy-astr.gsu.edu/hbase/pertab/perlewis.html
http://misterguch.brinkster.net/covalentcompounds.html
LEQ: How can I classify a bond type?
Electronegativity- how strong bonds are within a compound
Ionic bond- bonds between metals & non-metals; atoms with large differences in their tendencies to lose or gain electorns
Covalent bond- bonds between nonmetals & non-metals; atoms that have small differences in their tendencies to lose or gain electrons
Metallic bond- bonds between metals & metals; lose their valence electrons but do not gain them, so the electrons "flow" between the atoms (back & forth)
Polar- unequal distribution of electron density, the bond has partial negative & partial positive poles
Non-polar- atoms are identical, bonding pair is share equally
Organic compound- carbon is nearly always bonded to itself and hydrogen & often to other elements
Inorganic compound- any compund that does not contain carbon
Intermolecular force- the atrractive & repulsive forces among patricles in a sample of matter
http://www.chemteam.info/Bonding/Electroneg-Bond-Polarity.html
dept.sfcollege.edu/natsci/chem/chm2labs/BondTypes.pdf
http://staff.jccc.net/pdecell/chemistry/bonds.html
LEQ: How can I predict the 3-D shape of molecules?
Linear- 0 unbonded pairs around the central element
2 locations bonded to central
Hybridization: sp
Trigonal Planar- 0 unbonded pairs around central element
3 locations bonded to central
Hybridization: sp2
Bent- 2 unbonded paris around central element
2 locations bonded to central
Hybridization: sp3
Pyramidal- 1 unbonded pari around central element
3 locations bonded to central
Hybridization: sp3
Tetrahedral- 0 unbonded pairs around central element
4 locations bonded to central
Hybridization: sp3
Bond angle- the angle formed by the nuclei of two surrounding atoms with nucleus of the central atom at the vertex
VESPR model- predicts the 3-D shape of a molecule
http://www2.chemistry.msu.edu/faculty/reusch/VirtTxtJml/intro3.htm
http://library.thinkquest.org/C006669/data/Chem/bonding/shapes.html
http://intro.chem.okstate.edu/1314f00/lecture/chapter10/vsepr.html